Write down the ground state electron configuration of boron and give a set of quantum numbers that uniquely defines each electron. Show work

The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from those for H by changing the atomic number to Z=2 . Calculate the average distance of the electron from the nucleus in the 2s orbital and in the 2p orbital. Compare your results with those in Problem 11 and explain the difference.

What experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?

Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.

Suppose that the spin quantum number did not exist, and therefore only one electron could occupy each orbital of a many-electron atom. Give the atomic numbers of the first three noble-gas atoms in this case.

Based on the trend shown in Figure 11.5, draw the probability distribution of a harmonic oscillator wavefunction that has a very high value of n. Explain how this is consistent with the correspondence principle.

Photoelectron spectroscopy studies have determined the orbital energies for fluorine atoms to be 1s689eV2s34eV2p12eV Estimate the value of Zeff for F in each of these orbitals.

Explain (in point form) how a ground state hydrogen atom can emit IR and then BLUE visible light when its electron has only been excited once.

Write noble gas core ground-state electron configurations for atoms of (a) calcium; (b) chromium; (c) lead.

Write noble gas core ground-state electron configurations for atoms of (a) sodium; (b) nickel; (c) copper.